The Kinetic Molecular Theory explains the behavior of moving particles. -if a gas obeys all parts of the kinetic molecular theory, the gas is idea. -Real gases exist in our world. -The more energy a particle has, the faster it moves. Ke= ½ MV2
*The phase of a substance depends on a battle between a substance depends on a battle between a substances kinetic energy and the strength of intermolecular forces.
Intermolecular Forces (weakest to strongest)
1) London dispersion forces- arise from the random movement of electrons.
2) Dipole-dipole forces- found only in polar molecules
- dipoles are always there, hense dipole-dipole is stronger.
3) Hydrogen bonding-
- strongest of the 3 intermolecular forces.
- exist in compounds where the Hydrogen is directly bonded to N, O, or F.
Pressure- a force exerted over a given area
Barometer- atmostpheric pressure Manometer- measures gas pressure
Boiling point- temperature at which the vapor pressure of a liquid is equal to the atmospheric pressure
Vapor pressure - is the pressure resulting from the evaporation of a liquid
Three Thermometers Showing the Freezing and Boiling Point of Water in Kelvin, Celsius and Fahrenheit
EXAMPLES-
1) The atmospheric pressure is 1.12 atm. Find gas B's pressure. 1.12 760 mm Hg = 851 mm Hg - 18
1 atm = 833 is the pressure
For that example problem, 760 comes from the conversion for 1 atmosphere. Then you just multiply 1.12 and 760 together, which equals 851 and then subtract 18, which is the height of the manometer is 18. The total then equals 833.
2) If the atmospheric pressure is 729 mm Hg, what is the pressure of Gas B?
729- 15 = 714 mm Hg
15 is the height of the gas in the manometer, you would just need to subtract that from the atmospheric pressure in order to get the final answer.
CHAPTER 10- States of Matter
Solids, liquids and gases
The Kinetic Molecular Theory explains the behavior of moving particles.
- if a gas obeys all parts of the kinetic molecular theory, the gas is idea.
- Real gases exist in our world.
- The more energy a particle has, the faster it moves. Ke= ½ MV2
*The phase of a substance depends on a battle between a substance depends on a battle between a substances kinetic energy and the strength of intermolecular forces.
Intermolecular Forces (weakest to strongest)
1) London dispersion forces- arise from the random movement of electrons.
2) Dipole-dipole forces- found only in polar molecules
- dipoles are always there, hense dipole-dipole is stronger.
3) Hydrogen bonding-
- strongest of the 3 intermolecular forces.
- exist in compounds where the Hydrogen is directly bonded to N, O, or F.
Pressure- a force exerted over a given area
Barometer- atmostpheric pressure Manometer- measures gas pressure
Boiling point- temperature at which the vapor pressure of a liquid is equal to the atmospheric pressure
Vapor pressure - is the pressure resulting from the evaporation of a liquid
EXAMPLES-
1) The atmospheric pressure is 1.12 atm. Find gas B's pressure. 1.12 760 mm Hg = 851 mm Hg - 18
1 atm = 833 is the pressure
For that example problem, 760 comes from the conversion for 1 atmosphere. Then you just multiply 1.12 and 760 together, which equals 851 and then subtract 18, which is the height of the manometer is 18. The total then equals 833.
2) If the atmospheric pressure is 729 mm Hg, what is the pressure of Gas B?
729- 15 = 714 mm Hg
15 is the height of the gas in the manometer, you would just need to subtract that from the atmospheric pressure in order to get the final answer.